Chemistry

Chemistry: The Central Science | 13th Edition | ISBN: 9780321910417 | Authors: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
New Search

Chemistry: The Central Science 13th Edition solutions

Get Unlimited Answers

Author: Theodore E. Brown; H. Eugene LeMay; Bruce E. Bursten; Catherine Murphy; Patrick Woodward; Matthew E. Stoltzfus
Publisher: Pearson
ISBN: 9780321910417
Buy the book

Select Chapter:

We have answers for this textbook’s questions
Check out the solutions to this books Chapter Problems

Chapter Problems

Chapter: Problem: 37E

Chemistry: The Central Science 13
The average pH of normal arterial blood is 7.40. At normal body temperature (37C), \(K_{W}=2.4 \times 10^{-14}\). Calculate \(\left[H^{+}\right],\left[O H^{-}\right]\), and pOH for blood at this temperature. Equation transcription: Text transcription: K_{W}=2.4 \times 10^{-14} [H^{+}],[O

Chapter: Problem: 38E

Chemistry: The Central Science 13
The pH Scale (Section) Carbon dioxide in the atmosphere dissolves in raindrops to produce carbonic acid , causing the pH of clean, unpolluted rain to range from about 5.2 to 5.6. What are the ranges of and in the raindrops?

Chapter: Problem: 39E

Chemistry: The Central Science 13
The pH Scale (Section) Addition of the indicator methyl orange to an unknown solution leads to a yellow color. The addition of bromothymol blue to the same solution also leads to a yellow color, (a) Is the solution acidic, neutral, or basic? (b) What is the range (in whole numbers) of possible pH val

Chapter: Problem: 40E

Chemistry: The Central Science 13
The pH Scale (Section) Addition of phenolphthalein to an unknown colorless solution does not cause a color change. The addition of bromothymol blue to the same solution leads to a yellow color, (a) Is the solution acidic, neutral, or basic? (b) Which of the following can you establish about the solut

Chapter: Problem: 41E

Chemistry: The Central Science 13
Strong Acids and Bases (Section) Is each of the following statements true or false? (a) All strong acids contain one or more H atoms, (b) A strong acid is a strong electrolyte, (c) A 1.0-M solution of a strong acid will have pH = 1.0.

Chapter: Problem: 42E

Chemistry: The Central Science 13
Strong Acids and Bases (Section) Determine whether each of the following is true or false: (a) All strong bases are salts of the hydroxide ion. (b) The addition of a strong base to water produces a solution of pH > 7.0. (c) Because is not very soluble, it cannot be a strong base.

Chapter: Problem: 43E

Chemistry: The Central Science 13
Strong Acids and Bases (Section) Calculate the pH of each of the following strong acid solutions: (a) , (b) in 575 rnL of solution, (c) 5.00 rnL of 0.250 M diluted to 50.0 rnL, (d) a solution formed by mixing 10.0 rnL of 0.100 M HBr with 20.0 rnL of 0.200 M HCI.

Chapter: Problem: 44E

Chemistry: The Central Science 13
Calculations for a Weak Acid-Strong Base Titration Calculate the pH of the solution formed when 45.0 mL of 0.100 M NaOH is added to 50.0 mL of . If you think carefully about what happens during the course of a weak acid-strong base titration, you can learn some very interesting things. For example,

Chapter: Problem: 45E

Chemistry: The Central Science 13
Problem 45E Strong Acids and Bases (Section) Calculate [OH-] and pH for (a) 1.5 x 10-3M Sr(OH)2, (b) 2.250 g of LiOH in 250.0 rnL of solution, (c) 1.00 rnL of 0.175 M NaOH diluted to 2.00 L, (d) a solution formed by adding 5.00 rnL of 0.105 M KOH to 15.0 rnL of 9.5 x 10-2 M Ca(OH)2.

Chapter: Problem: 46E

Chemistry: The Central Science 13
Why is pH at the equivalence point larger than 7 when you titrate a weak acid with a strong base? (a) There is excess strong base at the equivalence point., (b) There is excess weak acid at the equivalence point.. (c) The conjugate base that is formed at the equivalence point is a strong base.. (d) T

Chapter: Problem: 47E

Chemistry: The Central Science 13
Problem 47E Strong Acids and Bases (Section) Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.50.

Chapter: Problem: 48E

Chemistry: The Central Science 13
Strong Acids and Bases (Section) Calculate the concentration of an aqueous solution of that has a pH of 10.05.

Chapter: Problem: 49E

Chemistry: The Central Science 13
Writing Solubility-Product (Ksp) Expressions Write the expression for the solubility-product constant for , and look up the corresponding Ksp value in Appendix D. Give the solubility-product-constant expressions and Ksp values (from Appendix D) for (a) barium carbonate and, (b) silver sulfate.

Chapter: Problem: 50E

Chemistry: The Central Science 13
Problem 50E Weak Acids (Section) Write the chemical equation and the Ka expression for the acid dissociation of each of the following acids in aqueous solution. First show the reaction with H+{aq) as a product and then with the hydroniurn ion: (a) C6H5COOH, (b) HC03-.

Chapter: Problem: 51E

Chemistry: The Central Science 13
Weak Acids (Section) Lactic acid has one acidic hydrogen. A 0.10 M solution of lactic acid has a pH of 2.44. Calculate Ka.

Chapter: Problem: 52E

Chemistry: The Central Science 13
Problem 52E Weak Acids (Section) Phenylacetic acid (C6H5CH2COOH) is one of the substances that accumulates in the blood of people with phenylketonuria, an inherited disorder that can cause mental retardation or even death. A 0.085 M solution of C6H5CH2COOH has a pH of 2.68. Calculate the Ka value

Chapter: Problem: 53E

Chemistry: The Central Science 13
A 0.100 M solution of chloroacetic acid is 11.0% ionized. Using this information, calculate , , and for chloroacetic acid.

Chapter: Problem: 54E

Chemistry: The Central Science 13
A 0.100 M solution of bromoacetic acid \(\left[B r C H_{2} C O O H\right]\) is 13.2% ionized. Calculate \(\left[H^{+}\right]\), \(\left[\mathrm{BrCH}_{2} \mathrm{COO}^{-}\right]\), \(\left[B r C H_{2} C O O H\right]\) and \(K_{a}\) for bromoacetic acid. Equation transcription: Text transcri

Chapter: Problem: 55E

Chemistry: The Central Science 13
Weak Acids (Section) A particular sample of vinegar has a pH of 2.90. If acetic acid is the only acid that vinegar contains , calculate the concentration of acetic acid in the vinegar.

Chapter: Problem: 56E

Chemistry: The Central Science 13
Problem 56E Weak Acids (Section) If a solution of HF (Ka = 6.8 x 10-4) has a pH of 3.65, calculate the concentration of hydrofluoric acid.

Chapter: Problem: 58E

Chemistry: The Central Science 13
Weak Acids (Section) The acid-dissociation constant for chlorous acid is . Calculate the concentrations of and at equilibrium if the initial concentration of is 0.0125 M.

Chapter: Problem: 57E

Chemistry: The Central Science 13
Weak Acids (Section) The acid-dissociation constant for benzoic acid is . Calculate the equilibrium concentrations of , and in the solution if the initial concentration of is 0.050 M.

Chapter: Problem: 59E

Chemistry: The Central Science 13
Problem 59E Weak Acids (Section) Calculate the pH of each of the following solutions (Ka and Kb values are given in Appendix D): (a) 0.095 M propionic acid (C2H5COOH), (b) 0.100 M hydrogen chromate ion (HCr04-), (c) 0.120 M pyridine (C5H5N).

Chapter: Problem: 60E

Chemistry: The Central Science 13
Problem 60E Weak Acids (Section) Determine the pH of each of the following solutions ( Ka and Kb values are given in Appendix D): (a) 0.095 M hypochlorous acid, (b) 0.0085 M hydrazine, (c) 0.165 M hydroxylamine.

Chapter: Problem: 61E

Chemistry: The Central Science 13
Saccharin, a sugar substitute, is a weak acid with \(p K_{a}=2.32\) at 25C. It ionizes in aqueous solution as follows: \(H N C_{7} H_{4} S O_{3}(a q) \leftrightarrow H^{+}(a q)+N C_{7} H_{4} S O_{3}^{-}(a q)\) What is the pH of a 0.10 M solution of this substance? Equation transcription: Tex

Chapter: Problem: 62E

Chemistry: The Central Science 13
Problem 62E Weak Acids (Section) The active ingredient in aspirin is acetylsalicylic acid (HC9H704), a rnonoprotic acid with Ka = 3.3 x 10-4 at 25 C. What is the pH of a solution obtained by dissolving two extra-strength aspirin tablets, containing 500 mg of acetylsalicylic acid each, in 250 rnl_

Chapter: Problem: 63E

Chemistry: The Central Science 13
Problem 63E Weak Acids (Section) Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations (Ka is given in Appendix D): (a) 0.400 W, (b) 0.100 W. (c) 0.0400 M.

Chapter: Problem: 64E

Chemistry: The Central Science 13
Problem 64E Weak Acids (Section) Calculate the percent ionization of propionic acid (C2H5COOH) in solutions of each of the following concentrations (Ka is given in Appendix D): (a) 0.250 M, (b) 0.0800 M, (c) 0.0200 M.

Chapter: Problem: 65E

Chemistry: The Central Science 13
Citric acid, which is present in citrus fruits, is a triprotic acid (Table 16.3). (a) Calculate the pH of a 0.040 M solution of citric acid. (b) Did you have to make any approximations or assumptions in completing your calculations? (c) Is the concentration of citrate ion \(\left(C_{6} H_{5} O_{7}^{3

Chapter: Problem: 66E

Chemistry: The Central Science 13
Tartaric acid is found in many fruits, including grapes, and is partially responsible for the dry texture of certain wines. Calculate the pH and the tartrate ion \(\left(C_{4} H_{4} O_{6}^{2-}\right)\) concentration for a 0.250 M solution of tartaric acid, for which the acid-dissociation constants ar

Chapter: Problem: 67E

Chemistry: The Central Science 13
Problem 67E Weak Bases (Section) Consider the base hydroxylamine, NH20H. (a) What is the conjugate acid of hydroxylamine? (b) When it acts as a base, which atom in hydroxylamine accepts a proton? (c) There are two atoms in hydroxylamine that have nonbonding electron pairs that could act as proton

Chapter: Problem: 68E

Chemistry: The Central Science 13
Problem 68E Weak Bases (Section) The hypochlorite ion, CIO-, acts as a weak base, (a) Is CIO- a stronger or weaker base than hydroxylamine? (b) When ClO acts as a base, which atom, Cl or O, acts as the proton acceptor? (c) Can you use formal charges to rationalize your answer to part (b)?

Chapter: Problem: 69E

Chemistry: The Central Science 13
Write the chemical equation and the \(K_{b}\) expression for the reaction of each of the following bases with water: (a) dimethylamine, \(\left(\mathrm{CH}_{3}\right) \mathrm{NH}\); (b) carbonate ion, \(\mathrm{CO}_{3}^{2-}\) (c) formate ion, \(\mathrm{CHO}_{2}^{-}\) Equation transcription:

Chapter: Problem: 70E

Chemistry: The Central Science 13
Problem 70E Weak Bases (Section) Write the chemical equation and the Kb expression for the reaction of each of the following bases with water: (a) propylamine, C3H7NH2; (b) monohydrogen phosphate ion, HP042-; (c) benzoate ion, C6H5C02-

Chapter: Problem: 71E

Chemistry: The Central Science 13
Problem 71E Weak Bases (Section) Calculate the molar concentration of OH- in a 0.075 M solution of ethylamine (C2H5NH2; Kb 6.4 x 10-4). Calculate the pH of this solution.

Chapter: Problem: 73E

Chemistry: The Central Science 13
Problem 73E Weak Bases (Section) Ephedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a weak organic Base: C10H15ON(aq) + H2O(l) ? C10H15ONH+(aq) + OH-(aq) A 0.035 M solution of ephedrine has a pH of 11.33. (a) What are the equilibrium c

Chapter: Problem: 72E

Chemistry: The Central Science 13
Problem 72E Weak Bases (Section) Calculate the molar concentration of OH- in a 0.724 M solution of hypobromite ion (BrO-; Kb = 4.0 x 10-6). What is the pH of this solution?

Chapter: Problem: 74E

Chemistry: The Central Science 13
Problem 74E Weak Bases (Section) Codeine (C18H21N03) is a weak organic base. A 5.0 x 10-3M solution of codeine has a pH of 9.95. Calculate the value of Kb for this substance. What is the pKb for this base?

Chapter: Problem: 75E

Chemistry: The Central Science 13
Problem 75E The Ka- Kb Relationship; Acid-Base Properties of Salts (Sections) Although the acid-dissociation constant for phenol (C6H50H) is listed in Appendix D, the base-dissociation constant for the phenolate ion (C6H50-) is not. (a) Explain why it is not necessary to list both Ka for phenol a

Chapter: Problem: 76E

Chemistry: The Central Science 13
Use the acid-dissociation constants in Table 16.3 to arrange these oxyanions from strongest base to weakest: \(S O_{4}^{2-}\), \(\mathrm{CO}_{3}^{2-}\), \(\mathrm{SO}_{3}^{2-}\), and \(P O_{4}^{3-}\). Equation transcription: Text transcription: S O_{4}^{2-} {CO}_{3}^{2-} {SO}_{3}^{2-} P O_{4}

Chapter: Problem: 78E

Chemistry: The Central Science 13
Problem 78E The Ka- Kb Relationship; Acid-Base Properties of Salts (Sections) (a) Given that Kb for ammonia is 1.8 X 10-5 and that for hydroxylamine is 1.1 X 10-8, which is the stronger base? (b) Which is the stronger acid, the arnrnoniurn ion or the hydroxylammonium ion? (c) Calculate Ka values

Chapter: Problem: 77E

Chemistry: The Central Science 13
Problem 77E The Ka- Kb Relationship; Acid-Base Properties of Salts (Sections) (a) Given that Ka for acetic acid is 1.8 x 10-5 and that for hypochlorous acid is 3.0 x 10-8, which is the stronger acid? (b) Which is the stronger base, the acetate ion or the hypochlorite ion? (c) Calculate Kb values

Chapter: Problem: 80E

Chemistry: The Central Science 13
Problem 80E The Ka- Kb Relationship; Acid-Base Properties of Salts (Sections) Using data from Appendix D, calculate [OH-] and pH for each of the following solutions: (a) 0.105 M NaF, (b) 0.035 M Na2S, (c) a mixture that is 0.045 M in NaCH3COO and 0.055 M in Ba(CH3COO)2.

Chapter: Problem: 81E

Chemistry: The Central Science 13
Problem 81E The Ka- Kb Relationship; Acid-Base Properties of Salts (Sections) A solution of sodium acetate (NaCH3COO) has a pH of 9.70. What is the molarity of the solution?

Chapter: Problem: 82E

Chemistry: The Central Science 13
Problem 82E The Ka- Kb Relationship; Acid-Base Properties of Salts (Sections) Pyridinium bromide (C5H5NHBr) is a strong electrolyte that dissociates completely into C5H5NH+ and Br-. A solution of pyridinium bromide has a pH of 2.95. What is the molarity of the solution?

Chapter: Problem: 83E

Chemistry: The Central Science 13
Problem 83E The Ka- Kb Relationship; Acid-Base Properties of Salts (Sections) Predict whether aqueous solutions of the following compounds are acidic, basic, or neutral: (a) NH4Br, (b) FeCL3, (c) Na2C03, (d) KCI04, (e) NaHC 204.

Chapter: Problem: 84E

Chemistry: The Central Science 13
Problem 84E The Ka- Kb Relationship; Acid-Base Properties of Salts (Sections) Predict whether aqueous solutions of the following substances are acidic, basic, or neutral: (a) AICI3, (b) NaBr, (c) NaCIO, (d) [CH3NH3]N03, (e) Na2S03.

Chapter: Problem: 85E

Chemistry: The Central Science 13
Problem 85E The Ka- Kb Relationship; Acid-Base Properties of Salts (Sections) An unknown salt is either NaF, NaCI, or NaOCI. When 0.050 mol of the salt is dissolved in water to form 0.500 L of solution, the pH of the solution is 8.08. What is the identity of the salt?

Chapter: Problem: 86E

Chemistry: The Central Science 13
Problem 86E The Ka- Kb Relationship; Acid-Base Properties of Salts (Sections) An unknown salt is either KBr, NH4Cl, KCN, or K2CO3. If a 0.100 M solution of the salt is neutral, what is the identity of the salt?

Chapter: Problem: 87E

Chemistry: The Central Science 13
Problem 87E Acid-Base Character and Chemical Structure (Section) Explain the following observations: (a) HN03 is a stronger acid than HN02; (b) H2S is a stronger acid than H20; (c) H2S04 is a stronger acid than HS04-; (d) H2S04 is a stronger acid than H2Se04; (e) CCI3COOH is a stronger acid than

Chapter: Problem: 88E

Chemistry: The Central Science 13
Problem 88E Acid-Base Character and Chemical Structure (Section) Explain the following observations: (a) HCI is a stronger acid than H2S; (b) H3P04 is a stronger acid than H3As04; (c) HE>r03 is a stronger acid than HE>r02; (d) H2C204 is a stronger acid than HC204 (e) benzoic acid (C6H5COOH

Chapter: Problem: 89E

Chemistry: The Central Science 13
Based on their compositions and structures and on conjugate acidbase relationships, select the stronger base in each of the following pairs: (a) \(\mathrm{BrO}^{-}\) or \(\mathrm{CIO}^{-}\), (b) \(\mathrm{BrO}^{-}\) or \(\mathrm{BrO}_{2}^{-}\), (c) \(\mathrm{HPO}_{4}^{2-}\) or \(\mathrm{H}_{2} \mathr

Chapter: Problem: 90E

Chemistry: The Central Science 13
Problem 90E Acid-Base Character and Chemical Structure (Section) Based on their compositions and structures and on conjugate acid-base relationships, select the stronger base in each of the following pairs: (a) N03- or N02-, (b) P04 3- or As043-, (c) HC03-or C032-.

Chapter: Problem: 91E

Chemistry: The Central Science 13
Problem 91E Acid-Base Character and Chemical Structure (Section) Indicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true, (a) In general, the acidity of binary acids increases from left to right in a given row of

Chapter: Problem: 92E

Chemistry: The Central Science 13
Problem 92E Acid-Base Character and Chemical Structure (Section) Indicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true, (a) Acid strength in a series of HA molecules increases with increasing size of A. (b) For

Chapter: Problem: 93E

Chemistry: The Central Science 13
Problem 93E Lewis Acids and Bases (Section) If a substance is an Arrhenius base, is it necessarily a Bronsted-Lowry base? Is it necessarily a Lewis base?

Chapter: Problem: 94E

Chemistry: The Central Science 13
Problem 94E If a substance is a Lewis acid, is it necessarily a Bronsted-Lowry acid? Is it necessarily an Arrhenius acid?

Chapter: Problem: 95E

Chemistry: The Central Science 13
Problem 95E Lewis Acids and Bases (Section) Identify the Lewis acid and Lewis base among the reactants in each of the following reactions: (a) Fe(ClO4)3(s) + 6 H2O(l) ? Fe(H2O)63+(aq) + 3 ClO4-(aq) (b) CN-(aq) + H2O(l) ? HCN(aq) + OH-(aq) (c) (CH3)3N(g) + BF3(g) ? (CH3)3NBF3(s) (d) HlO(lq

Chapter: Problem: 96E

Chemistry: The Central Science 13
Identify the Lewis acid and Lewis base in each of the following reactions: (a) \(\mathrm{HNO}_{2}(a q)+\mathrm{OH}^{-}(a q) \leftrightarrow \mathrm{NO}_{2}^{-}(a q)+\mathrm{H}_{2} \mathrm{O}(I)\) (b) \(F e B r_{3}(s)+B r^{-}(a q) \leftrightarrow F e B r_{4}^{-}(a q)\) (c) \(Z n^{2+}(a q)+4 N H_{3}(a

Chapter: Problem: 97E

Chemistry: The Central Science 13
Predict which member of each pair produces the more acidic aqueous solution: (a) \(K^{+}\) or \(C u^{2+}\), (b) \(\mathrm{Fe}^{2+}\) or \(\mathrm{Fe}^{3+}\), (c) \(A I^{3+}\) or \(G a^{3+}\). Equation transcription: Text transcription: K^{+} C u^{2+} {Fe}^{2+} {Fe}^{3+} A I^{3+} G a^{3+}

Chapter: Problem: 98E

Chemistry: The Central Science 13
Problem 98AE Lewis Acids and Bases (Section) Which member of each pair produces the more acidic aqueous solution: (a) ZnBr2 or CdCI2, (b) CuCI or Cu(N03)2, (c) Ca(N03)2 or NiBr2?

Chapter: Problem: 99AE

Chemistry: The Central Science 13
Problem 99AE Indicate whether each of the following statements is correct or incorrect. (a) Every Bronsted-Lowry acid is also a Lewis acid. (b) Every Lewis acid is also a Bronsted-Lowry acid. (c) Conjugate acids of weak bases produce more acidic solutions than conjugate a

Chapter: Problem: 100AE

Chemistry: The Central Science 13
Problem 100AE A solution is made by adding 0.300 g Ca(OH)2(s), 50.0 rnL of 1.40 M HN03, and enough water to make a final volume of 75.0 rnL Assuming that all of the solid dissolves, what is the pH of the final solution?

Chapter: Problem: 101AE

Chemistry: The Central Science 13
Problem 101AE The odor of fish is due primarily to amines, especially rnethylarnine (CH3NH2). Fish is often served with a wedge of lemon, which contains citric acid. The arnine and the acid react forming a product with no odor, thereby making the less-than-fresh fish more appetizing. Using data fro

Chapter: Problem: 102AE

Chemistry: The Central Science 13
Problem 102AE For solutions of a weak acid, a graph of pH versus the logarithm of the initial acid concentration should be a straight line. What is the magnitude of the slope of that line?

Chapter: Problem: 103AE

Chemistry: The Central Science 13
Problem 103AE Hemoglobin plays a part in a series of equilibria involving protonation-deprotonation and oxygenation-deoxygenation. The overall reaction is approximately as follows HbH + (aq) + O2(aq) ? HbO2(aq) + H + (aq) where Hb stands for hemoglobin and Hb02 for oxyhemoglobin, (a) The concen

Chapter: Problem: 104AE

Chemistry: The Central Science 13
Problem 104AE Calculate the pH of a solution made by adding 2.50 g of lithium oxide (Li20) to enough water to make 1.500 L of solution.

Chapter: Problem: 105AE

Chemistry: The Central Science 13
Benzoic acid \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH}\right) and aniline \(\left(C_{6} H_{5} N H_{2}\right)\) are both derivatives of benzene. Benzoic acid is an acid with \(K_{a}=6.3 \times 10^{-5}\) and aniline is a base with \(K_{a}=4.3 \times 10^{-10}\). (a) What are the conj

Chapter: Problem: 106AE

Chemistry: The Central Science 13
Problem 106AE What is the pH of a solution that is 2.5 x 10-9 M in NaOH? Does your answer make sense? What assumption do we normally make that is not valid in this case?

Chapter: Problem: 107AE

Chemistry: The Central Science 13
Problem 107AE Oxalic acid (H2C204) is a diprotic acid. By using data in Appendix D as needed, determine whether each of the following statements is true: (a) H2C204 can serve as both a Bronsted-Lowry acid and a Bronsted-Lowry base, (b) C204 2- is the conjugate base of HC204-. (c) An aqueous solution

Chapter: Problem: 108AE

Chemistry: The Central Science 13
Succinic acid \(\left(\mathrm{H}_{2} \mathrm{C}_{4} \mathrm{H}_{6} \mathrm{O}_{4}\right)\), which we will denote \(\mathrm{H}_{2} \mathrm{Suc}\), is a biologically relevant diprotic acid with the structure shown below. It is closely related to tartaric acid and malic acid (Figure 16.1). At \(25^{\cir

Chapter: Problem: 109AE

Chemistry: The Central Science 13
Problem 109AE Butyric acid is responsible for the foul smell of rancid butter. The pKa of butyric acid is 4.84. (a) Calculate the pKb for the butyrate ion. (b) Calculate the pH of a 0.050 M solution of butyric acid, (c) Calculate the pH of a 0.050 M solution of sodium butyrate.

Chapter: Problem: 110AE

Chemistry: The Central Science 13
Problem 110AE Arrange the following 0.10 M solutions in order of increasing acidity (decreasing pH): (i) NH4N03, (ii) NaN03, (iii) CH3COONH4, (iv) NaF, (v) CH3COONa.

Chapter: Problem: 111AE

Chemistry: The Central Science 13
Problem 111AE A 0.25 M solution of a salt Na A has pH = 9.29. What is the value of Ka for the parent acid HA?

Chapter: Problem: 112AE

Chemistry: The Central Science 13
Problem 112AE The following observations are made about a diprotic acid H2A: (i) A 0.10 M solution of H2A has pH = 3.30. (ii) A 0.10 M solution of the salt NaHA is acidic. Which of the following could be the value of pKa2 for H2A: (i) 3.22, (ii) 5.30, (iii) 7.47, or (iv) 9.32?

Chapter: Problem: 113AE

Chemistry: The Central Science 13
Problem 113AE Many moderately large organic molecules containing basic nitrogen atoms are not very soluble in water as neutral molecules, but they are frequently much more soluble as their acid salts. Assuming that pH in the stomach is 2.5, indicate whether each of the following compounds would be

Chapter: Problem: 114AE

Chemistry: The Central Science 13
The amino acid glycine (H2N?CH2?COOH) can participate in the following equilibria in water: \(H_{2}-C H_{2}-C O O H+H_{2} O \leftrightarrow H_{2} N-C H_{2}-\mathrm{COO}^{-}+H_{3} O^{+}\) \(K_{a}=4.3 x 10^{-3}\) \(H_{2}-\mathrm{CH}_{2}-\mathrm{COOH}+{ }^{+} \mathrm{H}_{3} \mathrm{~N}-\mathrm{C

Chapter: Problem: 115AE

Chemistry: The Central Science 13
The structural formula for acetic acid is shown in Table 16.2. Replacing hydrogen atoms on the carbon with chlorine atoms causes an increase in acidity, as follows: Using Lewis structures as the basis of your discussion, explain the observed trend in acidities in the series. Calculate the pH of a

Chapter: Problem: 116AE

Chemistry: The Central Science 13
Problem 116AE Calculate the number of ions in 1.0 mL of pure water at 25 C

Chapter: Problem: 117IE

Chemistry: The Central Science 13
Problem 117IE How many milliliters of concentrated hydrochloric acid solution (36.0% HCI by mass, density = 1.18 g/mL) are required to produce 10.0 L of a solution that has a pH of 2.05?

Chapter: Problem: 118IE

Chemistry: The Central Science 13
Problem 118IE The volume of an adults stomach ranges from about 50 mL when empty to 1 L when full. If the stomach volume is 400 mL and its contents have a pH of 2. how many moles of H+ does the stomach contain? Assuming that all the H+ comes from HCI. how many grams of sodium hydrogen carbonate wi

Chapter: Problem: 119IE

Chemistry: The Central Science 13
Problem 119IE Atmospheric C02 levels have risen by nearly 20% over the past 40 years from 315 ppm to 380 ppm. (a) Given that the average pH of clean, unpolluted rain today is 5.4, determine the pH of unpolluted rain 40 years ago. Assume that carbonic acid (H2C03) formed by the reaction of C02 and w

Chapter: Problem: 120IE

Chemistry: The Central Science 13
At 50C, the ion-product constant for \(\mathrm{H}_{2} \mathrm{O}\) has the value \(K_{W}=5.48 \times 10^{-14}\). (a) What is the pH of pure water at 50C? (b) Based on the change in \(K_{W}\) with temperature, predict whether ?H is positive, negative, or zero for the autoionization reaction of water:

Chapter: Problem: 121IE

Chemistry: The Central Science 13
Problem 121IE In many reactions the addition of A1CI3 produces the same effect as the addition of H+. (a) Draw a Lewis structure for AICI3 in which no atoms carry formal charges, and determine its structure using the VSEPR method, (b) What characteristic is notable about the structure in part (a) t

Chapter: Problem: 122IE

Chemistry: The Central Science 13
Problem 122IE What is the boiling point of a 0.10 M solution of NaHS04 if the solution has a density of 1.002 g/mL?

Chapter: Problem: 123IE

Chemistry: The Central Science 13
Use average bond enthalpies from Table 8.4 to estimate the enthalpies of the following gas-phase reactions: Reaction 1: \(H F(g)+H_{2} O(g) \leftrightarrow F^{-}(g)+H_{3} O^{+}(g)\) Reaction 2: \(H C I(g)+H_{2} O(g) \leftrightarrow C I^{-}(g)+H_{2} O^{+}(g)\) Are both reactions exothermic?

Chapter: Problem: 124IE

Chemistry: The Central Science 13
Problem 124IE Cocaine is a weak organic base whose molecular formula is C17H21N04. An aqueous solution of cocaine was found to have a pH of 8.53 and an osmotic pressure of 52.7 torr at 15 C. Calculate Kb for cocaine.

Chapter: Problem: 125IE

Chemistry: The Central Science 13
The iodate ion is reduced by sulfite according to the following reaction: \(I O_{3}^{-}(a q)+3 S O_{3}^{2-}(a q) \rightarrow I^{-}(a q)+3 S O_{4}^{2-}(a q)\) The rate of this reaction is found to be first order in \(\mathrm{IO}_{3}^{-}\), first order in \(\mathrm{SO}_{3}^{2-}\), and first ord

Chapter: Problem: 126IE

Chemistry: The Central Science 13
(a) Using dissociation constants from Appendix D, determine the value for the equilibrium constant for each of the following reactions. (i) \(\mathrm{HCO}_{3}^{-}(a q)+\mathrm{OH}^{-}(a q) \leftrightarrow \mathrm{CO}_{3}^{2-}(a q)+\mathrm{H}_{2} \mathrm{O}(\mathrm{I})\) (ii) \(\mathrm{NH}_{4}^{+}(a

Chapter: Problem: 79E

Chemistry: The Central Science 13
Problem 79E The Ka- Kb Relationship; Acid-Base Properties of Salts (Sections) Using data from Appendix D. calculate [OH-] and pH for each of the following solutions; (a) 0.10 M NaBrO. (b) 0.080 M NaHS. (c) a mixture that is 0.10 M in NaN02 and 0.20 M in Ca(N02)2.

Chapter: Problem: 1DE

Chemistry: The Central Science 13
Problem 1DE Your professor gives you a bottle that contains a clear liquid. You are told that the liquid is a pure substance that is volatile, soluble in water, and might be an acid or a base. Design experiments to elucidate the following about this unknown sample, (a) Determine whether the substan

Chapter: Problem: 1E

Chemistry: The Central Science 13
(a) Identify the BrnstedLowry acid and base in the reaction (b) Identify the Lewis acid and base in the reaction. [Sections 16.2 and 16.11]

Chapter: Problem: 2E

Chemistry: The Central Science 13
The following diagrams represent aqueous solutions of two monoprotic acids, HA (A = X or Y). The water molecules have been omitted for clarity. (a) Which is the stronger acid, HX or HY? (b) Which is the stronger base, \(X^{-}\) or \(Y^{-}\) ? (c) If you mix equal concentrations of HX and NaY, will th

Chapter: Problem: 3E

Chemistry: The Central Science 13
The indicator methyl orange has been added to both of the following solutions. Based on the colors, classify each statement as true or false: (a) The pH of solution A is definitely less than 7.00. (b) The pH of solution B is definitely greater than 7.00. (c) The pH of solution B is greater than that

Chapter: Problem: 4E

Chemistry: The Central Science 13
The probe of the pH meter shown here is sitting in a beaker that contains a clear liquid. (a) You are told the liquid is pure water, a solution of \(H C I(a q)\), or a solution of \(\mathrm{KOH}(a q)\). Which one is it? (b) If the liquid is one of the solutions, what is its molarity? (c) Why is the t

Chapter: Problem: 5E

Chemistry: The Central Science 13
The following diagrams represent aqueous solutions of three acids, HX, HY, and HZ. The water molecules have been omitted for clarity, and the hydrated proton is represented as H+ rather than \(\mathrm{H}_{3} \mathrm{O}^{+}\). (a) Which of the acids is a strong acid? Explain. (b) Which acid would have

Chapter: Problem: 6E

Chemistry: The Central Science 13
The graph given below shows \(\left[H^{+}\right]\) vs. concentration for an aqueous solution of an unknown substance. (a) Is the substance a strong acid, a weak acid, a strong base, or a weak base? (b) Based on your answer to (a), can you determine the value of the pH of the solution when the concent

Chapter: Problem: 7E

Chemistry: The Central Science 13
(a) Which of these three lines represents the effect of concentration on the percent ionization of a weak acid? (b) Explain in qualitative terms why the curve you chose has the shape it does. [Section 16.6]

Chapter: Problem: 8E

Chemistry: The Central Science 13
Each of the three molecules shown here contains an OH group, but one molecule acts as a base, one as an acid, and the third is neither acid nor base. (a) Which one acts as a base? Why does only this molecule act as a base? (b) Which one acts as an acid? (c) Why is the remaining molecule neither acidi

Chapter: Problem: 9E

Chemistry: The Central Science 13
Phenylephrine, an organic substance with molecular formula \(\mathrm{C}_{9} \mathrm{H}_{13} \mathrm{NO}_{2}\), is used as a nasal decongenstant in over-the-counter medications. The molecular structure of phenylephrine is shown below using the usual shortcut organic nomenclature. (a) Would you expect

Chapter: Problem: 10E

Chemistry: The Central Science 13
Which of the following diagrams best represents an aqueous solution of NaF? (For clarity, the water molecules are not shown.) Will this solution be acidic, neutral, or basic? [Section 16.9]

Chapter: Problem: 11E

Chemistry: The Central Science 13
Consider the molecular models shown here, where X represents a halogen atom. (a) If X is the same atom in both molecules, which molecule will be more acidic? (b) Does the acidity of each molecule increase or decrease as the electronegativity of the atom X increases? [Section 16.10]

Chapter: Problem: 12E

Chemistry: The Central Science 13
(a) The following diagram represents the reaction of \(P C I_{4}^{+}\) with Cl?. Draw the Lewis structures for the reactants and products, and identify the Lewis acid and the Lewis base in the reaction. (b) The following reaction represents a hydrated cation losing a proton. How does the equili

Chapter: Problem: 13E

Chemistry: The Central Science 13
Problem 13E Arrhenius and Bronsted-Lowry Acids and Bases (Sections) (a) What is the difference between the Arrhenius and the Bronsted-LowTy definitions of an acid? (b) NH3(g) and HCI(g) react to form the ionic solid NH4CI(s). Which substance is the Bronsted-Lowry acid in this reaction? Which is t

Chapter: Problem: 14E

Chemistry: The Central Science 13
Problem 14E Arrhenius and Bronsted-Lowry Acids and Bases (Sections) (a) What is the difference between the Arrhenius and the Bronsted-Lowiy definitions of a base? (b) Can a substance behave as an Arrhenius base if it does not contain an OH group? Explain. Step-by-step solution

Chapter: Problem: 15E

Chemistry: The Central Science 13
Problem 15E Arrhenius and Bronsted-Lowry Acids and Bases (Sections) (a) Give the conjugate base of the following Bronsted-Lowry acids:(i) HI03. (ii) NH4+. (b) Give the conjugate acid of the following Bronsted-Lowry bases: (i) 02-, (ii) H2P04-.

Chapter: Problem: 16E

Chemistry: The Central Science 13
Problem 16E Arrhenius and Bronsted-Lowry Acids and Bases (Sections) (a) Give the conjugate base of the following Brnsted-Lowry acids: (i) HCOOH, (ii) HPO42- (b) Give the conjugate acid of the following Brnsted-Lowry bases: (i) SO42-, (ii) CH3NH2.

Chapter: Problem: 18E

Chemistry: The Central Science 13
Problem 18E Arrhenius and Bronsted-Lowry Acids and Bases (Sections) Designate the Bronsted-Lowry acid and the Bronsted-Lowry base on the left side of each equation, and also designate the conjugate acid and conjugate base of each on the right side. (a) HBrO(aq) + H2O H3O+(aq) + BrO-(aq) (b) HSO

Chapter: Problem: 17E

Chemistry: The Central Science 13
Problem 17E Arrhenius and Bronsted-Lowry Acids and Bases (Sections) Designate the Bronsted-Lowry acid and the Bronsted-Lowry base on the left side of each of the following equations, and also designate the conjugate acid and conjugate base of each on the right side: (a) NH4+(aq) + CN-(aq) (b)

Chapter: Problem: 19E

Chemistry: The Central Science 13
Problem 19E Arrhenius and Bronsted-Lowry Acids and Bases (Sections) (a) The hydrogen sutfite ion (HS03-) is amphiprotic. Write a balanced chemical equation showing how it acts as an acid toward water and another equation showing how it acts as a base toward water, (b) What is the conjugate acid o

Chapter: Problem: 20E

Chemistry: The Central Science 13
Problem 20E Arrhenius and Bronsted-Lowry Acids and Bases (Sections) (a) Write an equation for the reaction in which H2C6H705 ~{aq) acts as a base in H20(I). (b) Write an equation for the reaction in which H2C6H705-(ag) acts as an acid in H20(I). (c) What is the conjugate acid of H2C6H705-(ag>)? W

Chapter: Problem: 21E

Chemistry: The Central Science 13
Problem 21E Arrhenius and Br0nsted-Lowry Acids and Bases (Sections) Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid,

Chapter: Problem: 22E

Chemistry: The Central Science 13
Problem 22E Arrhenius and Br0nsted-Lowry Acids and Bases (Sections) Label each of the following as being a strong acid, a weak acid, or a species with negligible acidity. In each case write the formula of its conjugate base, and indicate whether the conjugate base is a strong base, a weak base, o

Chapter: Problem: 23E

Chemistry: The Central Science 13
Problem 23E Arrhenius and Br0nsted-Lowry Acids and Bases (Sections) (a) Which of the following is the stronger Br0nsted-Lowry acid, HBrO or HBr? (b) Which is the stronger Br0nsted-Lowry base, F- or CI-?

Chapter: Problem: 24E

Chemistry: The Central Science 13
Problem 24E Arrhenius and Br0nsted-Lowry Acids and Bases (Sections) (a) Which of the following is the stronger Br0nsted-Lowry acid, HClO3 or HClO2? (b) Which is the stronger Br0nsted-Lowry base, HS- or HS04-?

Chapter: Problem: 25E

Chemistry: The Central Science 13
Problem 25E Arrhenius and Br0nsted-Lowry Acids and Bases (Sections) Predict the products of the following acid-base reactions, and predict whether the equilibrium lies to the left or to the right of the equation: (a) O2-(aq) + H2O(l) ? (b) CH3COOH(aq) + HS-(aq) ? (c) NO2-(aq) + H2O(l) ?

Chapter: Problem: 26E

Chemistry: The Central Science 13
Problem 26E Arrhenius and Br0nsted-Lowry Acids and Bases (Sections) Predict the products of the following acid-base reactions, and predict whether the equilibrium lies to the left or to the right of the equation: (a) NH4 + (aq) + OH-(aq) ? (b) CH3COO-(aq) + H3O+(aq)? (c) HCO3-(aq) + F-(aq)

Chapter: Problem: 27E

Chemistry: The Central Science 13
Problem 27E Autoionization of Water (Section) If a neutral solution of water, with pH = 7 00. is cooled to 10 C. the pH rises to 7.27. Which of the following three statements is correct for the cooled water (i) (H+) > [OH-], (ii) [H+]= [OH-], or (iii) [H+]<[OH-]?

Chapter: Problem: 28E

Chemistry: The Central Science 13
Problem 28E Autoionization of Water (Section) (a) Write a chemical equation that illustrates the autoionization of water, (b) Write the expression for the ion-product constant for water, Kw. (c) If a solution is described as basic, which of the following is true: (i) [H+]>[OH-], (ii) [H+] = [OH-]

Chapter: Problem: 29E

Chemistry: The Central Science 13
Problem 29E Autoionization of Water (Section) Calculate [H+] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) [OH-] = 0.00045 M; (b) [OH-] = 8.8 x 10-9 M; a solution in which [OH-] is 100 times greater than [H+]

Chapter: Problem: 30E

Chemistry: The Central Science 13
Problem 30E Autoionization of Water (Section) Calculate [OH-] for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) [H+] = 0.0505 M; (b) [H+] = 2.5 x 10-10 M; (c) a solution in which [H+] is 1000 times greater than [OH-].

Chapter: Problem: 31E

Chemistry: The Central Science 13
At the freezing point of water (0C), \(K_{w}=1.2 \times 10^{15}\). Calculate \(\left[H^{+}\right]\) and \(\left[\mathrm{OH}^{-}\right]\) for a neutral solution at this temperature. Equation transcription: Text transcription: Text transcription: K{w}=1.2 times 10^{15} [H^{+}] [{OH}^{-}]

Chapter: Problem: 32E

Chemistry: The Central Science 13
Problem 32E Autoionization of Water (Section) Deuterium oxide (D20, where D is deuterium, the hydrogen-2 isotope) has an ion-product constant, Kw, of 3.9 x 10-16 at 20 C. Calculate [D+] and [OD-] for pure (neutral) D20 at this temperature.

Chapter: Problem: 34E

Chemistry: The Central Science 13
Problem 34E The pH Scale (Section) Consider two solutions, solution A and solution B. [H+] in solution A is 250 times greater than that in solution B. What is the difference in the pH values of the two solutions?

Chapter: Problem: 33E

Chemistry: The Central Science 13
Problem 33E The pH Scale (Section) By what factor does [H+] change for a pH change of (a) 2.00 units, (b) 0.50 units?

Chapter: Problem: 35E

Chemistry: The Central Science 13
Complete the following table by calculating the missing entries and indicating whether the solution is acidic or basic.

Chapter: Problem: 36E

Chemistry: The Central Science 13
Complete the following table by calculating the missing entries. In each case indicate whether the solution is acidic or basic.

Chapter: Problem: 16.1a

Chemistry: The Central Science 13
(a) Identify the BrnstedLowry acid and base in the reaction + + = H = N = Cl +

Chapter: Problem: 16.1b

Chemistry: The Central Science 13
(b) Identify the Lewis acid and base in the reaction. [Sections 16.2 and 16.11]

Chapter: Problem: 16.2

Chemistry: The Central Science 13
The following diagrams represent aqueous solutions of two monoprotic acids, HA 1A = X or Y2. The water molecules have been omitted for clarity. (a) Which is the stronger acid, HX or HY? (b) Which is the stronger base, X- or Y-? (c) If you mix equal concentrations of HX and NaY, will the equilibrium H

Chapter: Problem: 16.3

Chemistry: The Central Science 13
The indicator methyl orange has been added to both of the following solutions. Based on the colors, classify each statement as true or false: (a) The pH of solution A is definitely less than 7.00. (b) The pH of solution B is definitely greater than 7.00. (c) The pH of solution B is greater than that

Chapter: Problem: 16.4

Chemistry: The Central Science 13
The probe of the pH meter shown here is sitting in a beaker that contains a clear liquid. (a) You are told the liquid is pure water, a solution of HCl(aq), or a solution of KOH(aq). Which one is it? (b) If the liquid is one of the solutions, what is its molarity? (c) Why is the temperature given on t

Chapter: Problem: 16.5

Chemistry: The Central Science 13
The following diagrams represent aqueous solutions of three acids, HX, HY, and HZ. The water molecules have been omitted for clarity, and the hydrated proton is represented as H+ rather than H3O+. (a) Which of the acids is a strong acid? Explain. (b) Which acid would have the smallest acid- dissociat

Chapter: Problem: 16.6

Chemistry: The Central Science 13
The graph given below shows 3H+4 vs. concentration for an aqueous solution of an unknown substance. (a) Is the substance a strong acid, a weak acid, a strong base, or a weak base? (b) Based on your answer to (a), can you determine the value of the pH of the solution when the concentration is 0.18 M?

Chapter: Problem: 16.7a

Chemistry: The Central Science 13
(a) Which of these three lines represents the effect of concentration on the percent ionization of a weak acid?

Chapter: Problem: 16.7b

Chemistry: The Central Science 13
(b) Explain in qualitative terms why the curve you chose has the shape it does. [Section 16.6] Acid concentration 0 0 Percent ionized C B A

Chapter: Problem: 16.8

Chemistry: The Central Science 13
Each of the three molecules shown here contains an OH group, but one molecule acts as a base, one as an acid, and the third is neither acid nor base. (a) Which one acts as a base? Why does only this molecule act as a base? (b) Which one acts as an acid? (c) Why is the remaining molecule neither acidi

Chapter: Problem: 16.9

Chemistry: The Central Science 13
Phenylephrine, an organic substance with molecular formula C9H13NO2, is used as a nasal decongenstant in over-thecounter medications. The molecular structure of phenylephrine is shown below using the usual shortcut organic nomenclature. (a) Would you expect a solution of phenylephrine to be acidic, n

Chapter: Problem: 16.10

Chemistry: The Central Science 13
Which of the following diagrams best represents an aqueous solution of NaF? (For clarity, the water molecules are not shown.) Will this solution be acidic, neutral, or basic? [Section 16.9] Solution A Na+ F OH HF Solution B Solution C + + + + + + + + + + + + + + + + +

Chapter: Problem: 16.11

Chemistry: The Central Science 13
Consider the molecular models shown here, where X represents a halogen atom. (a) If X is the same atom in both molecules, which molecule will be more acidic? (b) Does the acidity of each molecule increase or decrease as the electronegativity of the atom X increases? [Section 16.10] (a) (b) O O X H C

Chapter: Problem: 16.12a

Chemistry: The Central Science 13
(a) The following diagram represents the reaction of PCl4 + with Cl -. Draw the Lewis structures for the reactants and products, and identify the Lewis acid and the Lewis base in the reaction. + +

Chapter: Problem: 16.12b

Chemistry: The Central Science 13
(b) The following reaction represents a hydrated cation losing a proton. How does the equilibrium constant for the reaction change as the charge of the cation increases? [Sections 16.9 and 16.11] + + (n1)+ + n+

Chapter: Problem: 16.13a

Chemistry: The Central Science 13
(a) What is the difference between the Arrhenius and the BrnstedLowry definitions of an acid?

Chapter: Problem: 16.13b

Chemistry: The Central Science 13
(b) NH31g2 and HCl(g) react to form the ionic solid NH4Cl1s2. Which substance is the BrnstedLowry acid in this reaction? Which is the BrnstedLowry base?

Chapter: Problem: 16.14a

Chemistry: The Central Science 13
(a) What is the difference between the Arrhenius and the BrnstedLowry definitions of a base?

Chapter: Problem: 16.14b

Chemistry: The Central Science 13
(b) Can a substance behave as an Arrhenius base if it does not contain an OH group? Explain

Chapter: Problem: 16.15a

Chemistry: The Central Science 13
a) Give the conjugate base of the following BrnstedLowry acids: (i) HIO3, (ii) NH4 +.

Chapter: Problem: 16.15b

Chemistry: The Central Science 13
(b) Give the conjugate acid of the following BrnstedLowry bases: (i) O2-, (ii) H2PO4 -

Chapter: Problem: 16.16a

Chemistry: The Central Science 13
(a) Give the conjugate base of the following BrnstedLowry acids: (i) HCOOH, (ii) HPO4 2-

Chapter: Problem: 16.16b

Chemistry: The Central Science 13
(b) Give the conjugate acid of the following BrnstedLowry bases: (i) SO4 2-, (ii) CH3NH2.

Chapter: Problem: 16.17

Chemistry: The Central Science 13
Designate the BrnstedLowry acid and the BrnstedLowry base on the left side of each of the following equations, and also designate the conjugate acid and conjugate base of each on the right side: (a) NH4 +1aq2 + CN-1aq2 HCN1aq2 + NH31aq2 (b) 1CH323N1aq2 + H2O1l2 1CH323NH+1aq2 + OH- 1aq2 (c) HCOOH1aq2

Chapter: Problem: 16.18

Chemistry: The Central Science 13
Designate the BrnstedLowry acid and the BrnstedLowry base on the left side of each equation, and also designate the conjugate acid and conjugate base of each on the right side. (a) HBrO1aq2 + H2O1l2 H3O+1aq2 + BrO-1aq2 (b) HSO4 -1aq2 + HCO3 -1aq2 SO4 2 - 1aq2 + H2CO31aq2 (c) HSO3 -1aq2 + H3O+1aq2 H2S

Chapter: Problem: 16.19a

Chemistry: The Central Science 13
(a) The hydrogen sulfite ion 1HSO3 -2 is amphiprotic. Write a balanced chemical equation showing how it acts as an acid toward water and another equation showing how it acts as a base toward water.

Chapter: Problem: 16.19b

Chemistry: The Central Science 13
(b) What is the conjugate acid of HSO3 -? What is its conjugate base?

Chapter: Problem: 16.20a

Chemistry: The Central Science 13
(a) Write an equation for the reaction in which H2C6H7O5 -1aq2 acts as a base in H2O1l2.

Chapter: Problem: 16.20b

Chemistry: The Central Science 13
(b) Write an equation for the reaction in which H2C6H7O5 -1aq2 acts as an acid in H2O1l2.

Chapter: Problem: 16.20c

Chemistry: The Central Science 13
(c) What is the conjugate acid of H2C6H7O5 -1aq2? What is its conjugate base?

Chapter: Problem: 16.21

Chemistry: The Central Science 13
Label each of the following as being a strong base, a weak base, or a species with negligible basicity. In each case write the formula of its conjugate acid, and indicate whether the conjugate acid is a strong acid, a weak acid, or a species with negligible acidity: (a) CH3COO-, (b) HCO3 -, (c) O2-,

Chapter: Problem: 16.22